The solubility of $AgCl$ is $1.43 \times 10^{-3} \ g/L$. If the molar mass of $AgCl$ is $143 \ g/mol$,then the solubility product $(K_{sp})$ is:

Solubility product is

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$Ag_2CO_3 \downarrow + 2HCl \longrightarrow 2AgCl \downarrow + CO_2 \uparrow + H_2O$

The solubility product of magnesium hydroxide $Mg(OH)_2$ is $1.2 \times 10^{-11}$. Calculate its solubility in pure water and $0.05 \ M$ $NaOH$.

If the solubility product of $CaSO_4$ is $2.5 \times 10^{-5}$,then its solubility will be .......

$M_{3}A_{2}$ is a sparingly soluble salt of molar mass $y \text{ g mol}^{-1}$ and solubility $x \text{ g L}^{-1}$. The ratio of the molar concentration of the anion $(A^{3-})$ to the solubility product of the salt is